An organic compound A contain 62.0% by mass of carbon, 21.1% by mass of nitrogen, the reminder being hydrogen. Determine the percentage by mass of hydrogen and the empirical formula A.....Can any one help me on that?????
Take a 100 g sample. This will give you
62.0 g C
21.1 g N
100-21.1-62.0 = ?? g O
Now convert each of these grams into moles. moles = g/atomic mass.
The empirical formula consists of small whole numbers for the atoms; therefore, find the ratio of these moles to each other in small whole numbers. The easiest way to do that is to divide the smallest number by itself. That will make the smallest number 1.00. Divide the other values by the same small number. By the way, check the values in your post to make sure there is no typo. Second, is this a book problem or a lab problem?
Sure, I can help you with that! Let's start by calculating the percentage by mass of hydrogen in the compound A.
Given:
Mass of carbon = 62.0%
Mass of nitrogen = 21.1%
To determine the percentage of hydrogen, we need to subtract the mass percentages of carbon and nitrogen from 100% (since these are the only three elements in the compound).
Mass of hydrogen = 100% - (62.0% + 21.1%) = 100% - 83.1% = 16.9%
So, the compound A contains approximately 16.9% hydrogen by mass.
Now, to determine the empirical formula of the compound, we need to find the simplest whole-number ratio of the elements present.
To do this, we assume that we have 100 grams of compound A. This means we have 62.0 grams of carbon, 21.1 grams of nitrogen, and 16.9 grams of hydrogen.
Now let's convert the masses into moles:
Moles of carbon = 62.0 g / molar mass of carbon
Moles of nitrogen = 21.1 g / molar mass of nitrogen
Moles of hydrogen = 16.9 g / molar mass of hydrogen
Finally, divide each mole value by the smallest mole value obtained to find the whole-number ratio.
Let's say we find that the smallest mole value is x, then the mole ratios of carbon, nitrogen, and hydrogen would be:
Mole ratio of carbon:x
Mole ratio of nitrogen:y
Mole ratio of hydrogen:z
Therefore, the empirical formula of compound A would be CxNyHz, where x, y, and z represent the whole-number ratios we obtained.
I hope that helps! Let me know if you have any more questions.
To determine the percentage by mass of hydrogen, we need to subtract the mass percentages of carbon and nitrogen from 100%.
Given:
Mass percentage of carbon = 62.0%
Mass percentage of nitrogen = 21.1%
Mass percentage of hydrogen = 100% - (mass percentage of carbon + mass percentage of nitrogen)
Mass percentage of hydrogen = 100% - (62.0% + 21.1%)
Mass percentage of hydrogen = 100% - 83.1%
Mass percentage of hydrogen = 16.9%
Therefore, the compound A contains 16.9% hydrogen by mass.
To find the empirical formula of A, we need to determine the ratio of atoms present in the compound.
First, we need to convert the mass percentages into moles, assuming 100g of the compound.
Given:
Mass of carbon = 62.0g
Mass of nitrogen = 21.1g
Mass of hydrogen = 16.9g
Now, we calculate the number of moles using the molar mass of each element:
Molar mass of carbon (C) = 12.01 g/mol
Molar mass of nitrogen (N) = 14.01 g/mol
Molar mass of hydrogen (H) = 1.01 g/mol
Moles of carbon = Mass of carbon / Molar mass of carbon = 62.0g / 12.01 g/mol
Moles of nitrogen = Mass of nitrogen / Molar mass of nitrogen = 21.1g / 14.01 g/mol
Moles of hydrogen = Mass of hydrogen / Molar mass of hydrogen = 16.9g / 1.01 g/mol
Simplifying the ratios:
Moles of carbon = 5.164 moles
Moles of nitrogen = 1.50 moles
Moles of hydrogen = 16.73 moles
To determine the simplest whole-number ratio, we divide the moles of each element by the smallest number of moles (1.50 moles for nitrogen in this case):
Carbon: 5.164 moles / 1.50 moles = 3.443
Nitrogen: 1.50 moles / 1.50 moles = 1.00
Hydrogen: 16.73 moles / 1.50 moles = 11.15
Rounding the ratios to the nearest whole number gives us:
Carbon: 3
Nitrogen: 1
Hydrogen: 11
Therefore, the empirical formula of compound A is C3N1H11.
Sure, I can help you with that!
To determine the percentage by mass of hydrogen and the empirical formula of compound A, we need to follow a few steps.
Step 1: Determine the mass of each element present in the compound.
Given that compound A contains 62.0% carbon, 21.1% nitrogen, and the remainder is hydrogen, we can assume that the remaining percentage is hydrogen.
Let's assume we have 100 grams of compound A.
- The mass of carbon = 62.0% of 100 grams = 62.0 grams
- The mass of nitrogen = 21.1% of 100 grams = 21.1 grams
- The mass of hydrogen = 100 grams - (62.0 grams + 21.1 grams) = 16.9 grams
Step 2: Convert the mass of each element to moles.
To convert the mass of each element to moles, we need to divide the mass of each element by its molar mass. The molar mass is the mass of one mole of an element or molecule.
The molar masses are approximately:
- Carbon (C): 12.01 g/mol
- Nitrogen (N): 14.01 g/mol
- Hydrogen (H): 1.01 g/mol
- Moles of carbon = mass of carbon / molar mass of carbon
= 62.0 grams / 12.01 g/mol
≈ 5.16 mol
- Moles of nitrogen = mass of nitrogen / molar mass of nitrogen
= 21.1 grams / 14.01 g/mol
≈ 1.5 mol
- Moles of hydrogen = mass of hydrogen / molar mass of hydrogen
= 16.9 grams / 1.01 g/mol
≈ 16.7 mol
Step 3: Find the simplest whole number ratio of the elements.
To find the empirical formula, we need to divide the number of moles of each element by the smallest number of moles among them.
In this case, the smallest number of moles is approximately 1.5 mol (which corresponds to nitrogen).
- Carbon: 5.16 mol / 1.5 mol ≈ 3.44
- Nitrogen: 1.5 mol / 1.5 mol = 1
- Hydrogen: 16.7 mol / 1.5 mol ≈ 11.1
Since we want the simplest whole number ratio, we can round off the above values to the nearest whole number.
The empirical formula of compound A is C3H11N, which represents the simplest, whole number ratio of carbon, hydrogen, and nitrogen in the compound.
Step 4: Calculate the percentage by mass of hydrogen.
To determine the percentage by mass of hydrogen, we need to divide the mass of hydrogen by the total mass of the compound and then multiply by 100.
- Percentage by mass of hydrogen = (mass of hydrogen / total mass of compound) * 100
= (16.9 grams / 100 grams) * 100
= 16.9%
Therefore, the percentage by mass of hydrogen in compound A is approximately 16.9%.
I hope this helps! Let me know if you have any further questions.